H₂(g)+1₂(g) → 2 HI(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.5. The engineer charges ("fills") three reaction vessels with hydrogen and iodine, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A ere to search B с I Don't Know compound H₂ 1₂ HI H₂ 1₂ HI H₂ 12₂ HI Submit 481 pressure 3.40 atm 4.50 atm 3.67 atm 3.76 atm 5.11 atm 5.29 atm 2.61 atm 3.71 atm 5.24 atm M expected change in pressure increase O increase ↑ O ↑ increase O 1 increase O † increase O ↑ increase O↑ increase O 1 increase O ↑ increase O decrease O ↓ decrease O ↓ decrease OI decrease O ↓ decrease O decrease O1 decrease O decrease ↓ O ↓ decrease O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) a olo Ar © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility ? 38°F Rain showers 12:08 AM 2/13/2023 Ę
H₂(g)+1₂(g) → 2 HI(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.5. The engineer charges ("fills") three reaction vessels with hydrogen and iodine, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A ere to search B с I Don't Know compound H₂ 1₂ HI H₂ 1₂ HI H₂ 12₂ HI Submit 481 pressure 3.40 atm 4.50 atm 3.67 atm 3.76 atm 5.11 atm 5.29 atm 2.61 atm 3.71 atm 5.24 atm M expected change in pressure increase O increase ↑ O ↑ increase O 1 increase O † increase O ↑ increase O↑ increase O 1 increase O ↑ increase O decrease O ↓ decrease O ↓ decrease OI decrease O ↓ decrease O decrease O1 decrease O decrease ↓ O ↓ decrease O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) O (no change) a olo Ar © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility ? 38°F Rain showers 12:08 AM 2/13/2023 Ę
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The direction in which the reaction proceeds to reach equilibrium can be predicted by determining the reaction quotient at given partial pressure of Reaction species.
Reaction quotient is the product of the concentrations of the products, each raised to the power equal to a stoichiometric coefficient divided by the product of the concentrations of the reactant each raised to the power equal to its stoichiometric coefficient at a particular point of time.
If Qp > Kp , then the reaction will shift to the left i.e. towards reactants.
If Qp < Kp, then the reaction will shift to the right i.e. towards products.
If Qp = Kp, then the reaction is at equilibrium.
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